Lattice Energy Research Paper
Definition of lattice energy :
For an ionic compound the lattice enthalpy is the enthalpy change when one mole of solid in its standard state is formed from its ions in the gaseous state. It simple words, it can also be stated as the measure of the energy contained in the crystal lattice of an ionic solid , and is equal to the energy that would be released if the component ions were brought together from infinity. The process will always be exothermic, and thus the value for lattice energy will be negative. Its values are usually expressed with the units kJ/mol. The concept of Lattice Energy is used to explain the stability of ionic solids. Some might expect such an ordered structure could hamper stability because the entropy of the
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The ionic radii (it affects the distance between the ions).
The charges on the ions
If we take the example of sodium chloride and magnesium oxide , both of them have exactly the same arrangements of ions in the crystal lattice, but the lattice enthalpies differ to a great extent. The lattice enthalpy of NaCl is 786 kJmol-1 while the lattice enthalpy of MgO is 3795 kJ mol-1 which is much more than that of sodium chloride.
The reason behind such major difference is , the difference in charge of respective ions. In magnesium oxide, 2+ ions are attracting 2- ions, while in sodium chloride, the attraction is only between 1+ and 1- ions. Thus , creating a stark difference between lattice enthalpies of two compounds
.
Fig : difference in lattice enthalpies of sodium chloride and magnesium oxide
Note: In the above diagram, intereste has not been shown in whether the lattice enthalpy is defined as a positive or a negative number. Interest has only been shown in their relative sizes. The values are for lattice dissociation enthalpies. If you prefer lattice formation enthalpies , then putting a negative sign mentally in front of each number will do the
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